Homogeneous Aqueous Systems 15.2 An ordinary dill pickle from the deli can be a source of light! Iron or copper electrodes are inserted into the ends of the pickle and connected to a source of alternating electric current. You will learn what kind of solution conducts electricity.

15.2 Solvents and Solutes Solvents and Solutes What is the difference between a solvent and a solute?

An aqueous solution is water that contains dissolved substances. 15.2 Solvents and Solutes An aqueous solution is water that contains dissolved substances. In a solution, the dissolving medium is the solvent. In a solution, the dissolved particles are the solute.

Solvents and solutes may be gases, liquids, or solids. 15.2 Solvents and Solutes A solvent dissolves the solute. The solute becomes dispersed in the solvent. Solvents and solutes may be gases, liquids, or solids. Solute particles can be atoms, ions, or molecules.

15.2 Solvents and Solutes If you filter a solution through filter paper, both the solute and the solvent pass through the filter. A solution cannot be separated by filtration. The small size of the solute particles allows them to pass through filter paper.

The Solution Process What happens in the solution process? 15.2

15.2 The Solution Process As individual solute ions break away from the crystal, the negatively and positively charged ions become surrounded by solvent molecules, and the ionic crystal dissolves.

15.2 The Solution Process The process by which the positive and negative ions of an ionic solid become surrounded by solvent molecules is called solvation.

Solvation of an Ionic Solid 15.2 The Solution Process Solvation of an Ionic Solid When an ionic solid dissolves, the ions become solvated or surrounded by solvent molecules. Inferring Why do the water molecules orient themselves differently around the anions and the cations?

Nonpolar solvents such as gasoline dissolve nonpolar compounds. 15.2 The Solution Process Polar solvents such as water dissolve ionic compounds and polar compounds. Nonpolar solvents such as gasoline dissolve nonpolar compounds.

Oil and water do not mix. 15.2 The Solution Process Oil and water do not mix. Oil is less dense than water, so it floats on top. The colors result from the bending of light rays by the thin film of oil.

Simulation 18 Explore the nature of solute- solvent interactions. The Solution Process Simulation 18 Explore the nature of solute- solvent interactions.

Electrolytes and Nonelectrolytes 15.2 Electrolytes and Nonelectrolytes Electrolytes and Nonelectrolytes Why are all ionic compounds electrolytes?

Electrolytes and Nonelectrolytes 15.2 Electrolytes and Nonelectrolytes An electrolyte is a compound that conducts an electric current when it is in an aqueous solution or in the molten state. All ionic compounds are electrolytes because they dissociate into ions.

Electrolytes and Nonelectrolytes 15.2 Electrolytes and Nonelectrolytes The bright glow shows that sodium chloride is a strong electrolyte because nearly all the dissolved sodium chloride exists as separate Na+ and Cl– ions. A solution conducts electricity if it contains ions. a) Sodium chloride, a strong electrolyte, is nearly 100% dissociated into ions in water. b) Mercury(II) chloride, a weak electrolyte, is only partially dissociated in water. c) Glucose, a nonelectrolyte, does not dissociate in water.

Electrolytes and Nonelectrolytes 15.2 Electrolytes and Nonelectrolytes A weak electrolyte conducts electricity poorly because only a fraction of the solute in the solution exists as ions. A solution conducts electricity if it contains ions. a) Sodium chloride, a strong electrolyte, is nearly 100% dissociated into ions in water. b) Mercury(II) chloride, a weak electrolyte, is only partially dissociated in water. c) Glucose, a nonelectrolyte, does not dissociate in water.

Electrolytes and Nonelectrolytes 15.2 Electrolytes and Nonelectrolytes A compound that does not conduct an electric current in either aqueous solution or the molten state is called a nonelectrolyte. A solution conducts electricity if it contains ions. a) Sodium chloride, a strong electrolyte, is nearly 100% dissociated into ions in water. b) Mercury(II) chloride, a weak electrolyte, is only partially dissociated in water. c) Glucose, a nonelectrolyte, does not dissociate in water.

Electrolytes and Nonelectrolytes Simulation 19 Simulate the behavior of electrolytes and nonelectrolytes in a circuit and at the atomic level.

15.2 Hydrates Hydrates How do you write the formula for a hydrate?